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Kinetics/Equilibrium Test Review

Total questions: 34

Worksheet time: 33mins

Name
Class
Date
1.
What two factors govern whether a collision between reacting particles will be effective?
a)
orientation and potential energy 
b)
kinetic energy and temperature 
c)
kinetic energy and orientation 
d)
potential energy and kinetic energy 
2.
More collisions correspond to a: 
a)
Faster reaction rate  
b)
Slower reaction rate
c)
Constant reaction rate 
d)
None of the above
3.
Which of the following is NOT a factor affecting reaction rate?
a)
temperature
b)
catalysts
c)
particle size
d)
polarity
4.
Decreasing the particle size increases the reaction rate because
a)
It makes particles move faster
b)
It increases the likelihood of collisions with the correct geometry
c)
It decreases the surface area available to react
d)
It increases the number of collisions
5.
To slow down a chemical reaction you will do one of the following:
a)
Place the reactants in hot water
b)
Place the products in ice bath
c)
Place the reactants in a ice bath
d)
Keep stirring the reactants with a stirring rod
6.
Why does a higher temperature increase the rate of a reaction?
a)
it increases both the frequency and energy of particle collisions
b)
it only increases the frequency of particle collisions
c)
it only increases the energy of particle collisions
d)
it reduces the activation energy of the reaction
7.
Which of the following increase the reaction rate?
a)
less surface area
b)
lower temperature
c)
an inhibitor
d)
increased concentration
8.

What is activation energy?

a)

The maximum amount of energy used

b)

The minimum amount of energy required for a reaction to start

c)

The energy of the reactants

d)

The energy possessed by the products

9.
Limestone chunks are reaction with hydrochloric acid solution at constant temperature with average speed. If we crash the chunks of limestone into powder how would speed of reaction change?
a)
Reaction speeds up
b)
Reaction does not change
c)
Reaction slows down
d)
Reaction stops
10.

Which factors increase the rate of a reaction?

a)

increasing temperature

b)

increasing concentration

c)

increasing surface area

d)

all of the above

11.
Which letter corresponds to the activation energy of the forward reaction?
a)
A
b)
B
c)
C
d)
D
12.

Which of these will change the value of the equilibrium constant?

a)

Increasing the initial concentration of a reactant.

b)

Increasing the temperature of the system.

c)

Increasing the pressure for a gas phase reaction.

d)

All of these will change the equilibrium constant.

13.
Which of the following is NOT true at equilibrium?
a)
The forward and reverse reactions proceed at the same rate.
b)

The concentrations of reactants and products remain constant.

c)
The concentration of the reactants is equal to the concentration of the products.
d)

Interconversions between reactants and products still proceed.

14.

Select the equilibrium constant for the most reactant favored system.

a)

3.0×10−33.0\times10^{-3}  

b)

7.0×10−37.0\times10^{-3}  

c)

8.0×10−58.0\times10^{-5}  

d)

2.0×10−52.0\times10^{-5}  

15.

What is the equilibrium expression for:

Fe3O4(s) + 4H2(g) ⇄ 3Fe(s) + 4H2O(g)

Kc =

a)

[Fe]3[H2O]4[Fe3O4][H2]4\frac{\left[Fe\right]^3\left[H_2O\right]^4}{\left[Fe_3O_4\right]\left[H_2\right]^4}

b)

[H2]4[H2O]4\frac{\left[H_2\right]^4}{\left[H_2O\right]^4}

c)

[H2O]4[H2]4\frac{\left[H_2O\right]^4}{\left[H_2\right]^4}

d)

[Fe3O4][H2]4[Fe]3[H2O]4\frac{\left[Fe_3O_4\right]\left[H_2\right]^4}{\left[Fe\right]^3\left[H_2O\right]^4}

16.

For the reaction

N2 (g) + 3 H2(g) ⇄ 2 NH3 (g)


If the pressure in the system is increased, which substance(s) will have a higher conentration after equilibrum is reattained?

a)

all 3 gases

b)

N2 and H2

c)

NH3

d)

The concentrations wouldn't change.

17.

2 SO2(g) + O2(g) ⇄ 2 SO3(g)

Adding SO2(g) will

a)

shift equilibrium right

b)

shift equilibrium left

c)

increase Kc

d)

not cause a shift

18.

2 SO2(g) + O2(g) ⇄ 2 SO3(g)

Removing O2(g) will

a)

shift equilibrium right

b)

shift equilibrium left

c)

increase pressure

d)

have no change

19.

Decreasing the temperature of an endothermic reaction will cause

a)

equilibria to shift left and K increases

b)

equilibria to shift left and K decreases

c)

equilibria to shift right and K increases

d)

equilibria to shift right and K decreases

20.
Given the equation representing a reaction at equilibrium: 
N2(g) + 3H2(g) --> 2NH3(g) + energy
Which change causes the equilibrium to shift to the right?
a)
decreasing the concentration of H2(g)
b)
decreasing the pressure
c)
increasing the concentration of N2(g)
d)
increasing the temperature
21.

Which alteration will shift the equilibrium reaction below to form more reactants? NH4Cl + heat <-> NH3 + HCl

a)

Increase concentration of NH3 and HCl

b)

decrease concentration of NH3 and HCl

c)

increase the temperature

d)

add a catayst

22.
Given the reaction at equilibrium:
N2(g) + 3H2(g) ↔ 2NH3(g)
Increasing the concentration of N2(g) will increase the forward reaction rate due to
a)
a decrease in the number of effective collisions
b)
an increase in the number of effective collisions
c)
a decrease in the activation energy
d)
an increase in the activation energy
23.
Given the reaction at equilibrium:
N2(g) + O2(g) ↔ 2NO(g)
As the concentration of N2(g) is increased, the concentration of O2(g) will
a)
decrease
b)
increase
c)
remain the same
24.
2NH3+22kJ↔N2+3H2
Which direction does the reaction shift if N2 was removed?
a)
Shift right 
b)
Shift left
c)
No shift
d)
Shift both directions
25.
2NH3+22kJ↔N2+3H2
Which direction does the reaction shift if H2 was removed?
a)
Shift right 
b)
Shift left
c)
No shift
d)
Shift both directions
26.
At what time the reaction reached equilibrium?
a)
t1
b)
t2
c)
t3
d)
t4
27.
The idea that when a system at equilibrium is stressed, it will react to relieve that stress and return to equilibrium is known as:
a)
Boyle's Law
b)
Le Chatelier's Principle
c)
Charles Law
d)
Denninger's Law
28.

Consider the following reaction. What would be the equilibrium constant expression?

4Br2(g) + CH4(g) ↔ 4HBr(g) + CBr4(g)

a)

Kc = [Br2]4 [CH4]/ [HBr]4 [CBr4]

b)

Kc = [HBr]4 [CBr4]/ [Br2]4 [CH4]

c)

Kc = [HBr ]/ [Br2]4 [CH4]

d)

Kc = [HBr]4 [CBr4]/ [Br2]4 [CH]4

29.

What is the reaction/equation for this Kc expression

a)

2N2 + O2 ⇌ 2NO

b)

N2 + O2 ⇌ NO

c)

NO ⇌ 2NO

d)

N2 + O2 ⇌ 2NO

30.
N2O4(g) ↔ 2 NO2(g)
What is the concentration equilibrium constant expression?
a)
Kc = [NO2]2/[N2O4]
b)
Kc = [N2O4]/[NO2]2
c)
Kc = [N2O4]2/[NO2]
d)
Kc = [NO2]/[N2O4]2
31.
Two reactant particles collide with proper orientation.The collision will be effective if the particles have
a)
high activation energy
b)
high ionization energy
c)
sufficient kinetic energy
d)
sufficient potential energy
32.

Given the reaction:

CH4(g) + 2 O2(g) --> 2 H2O(g) + CO2(g)

What is the overall result when CH4(g) burns according to this reaction?

a)

Energy is absorbed and H is negative.Δ

b)

Energy is absorbed and ΔH is positive.

c)

Energy is released and ΔH is negative.

d)

Energy is released and ΔH is positive

33.

Temperature is a measure of average ________ energy of individual atoms.

a)

heat

b)

potential

c)

mechanical

d)

kinetic

34.

Given the equation representing a reaction at equilibrium:

N2(g) + 3H2(g) --> 2NH3(g) + energy

Which change causes the equilibrium to shift to the right?

a)

decreasing the concentration of H2(g)

b)

decreasing the pressure

c)

increasing the concentration of N2(g)

d)

increasing the temperature

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